Liquids supercooling

Fig. 1. Volume—temperature relationships for glasses, liquids, supercooled liquids, and crystals.

Mishima, O. and Stanley, H.E. 1998. The relationship between liquid, supercooled and glassy water. Nature 396, 329-335. 

Liquid, determination of density and refractive index of, 1029-1034 Liquid ammonia, reactions in, 895-902 Liquids, partially miscible, 17-19 Liquids, supercooled, 22, 23 Liquidus, 26, 33... 

Silicobromoform is a colorless, mobile liquid, boiling at 111.8°C. and freezing to a white solid melting at — 73.5°C. The liquid supercools to a remarkable degree. It is usually spontaneously inflammable when poured through the air. The vapor pressure at 0°C. is 8.8 mm. and may be expressed with an accuracy of a few tenths of a per cent by the equation ... 

Physical Properties.— The crystalline acid was found to melt at 70-1° C.,5 74° C.6 The density of the liquid supercooled at 21° C. was 1-651.5 The latent heat of fusion of the acid was found to be 7-07 Cals.5 The heat of solution of the acid per mol dissolved in 400 mols or more of water was +233 Cals.5 The heat of formation of the crystallised acid has been given as +227-7 Cals.5... 

When a liquid supercools (i.e., does not crystallize when its temperature drops below the thermodynamic melting point), the liquidlike structure is frozen due to the high viscosity of the system. The supercooled liquid is in a so-called viscoelastic state. If the crystallization can be further avoided as the ten ierature continues to drop, a glass transition will happen at a certain temperature, where the frozen liquid turns into a brittle, rigid state known as a glassy state. A well-accepted definition for glass transition is that the relaxation time t of the system is 2 X10 s or the viscosity / isio Pas (an arbitrary standard, of course). 

Fig. 19.1. Heat capacity of glycerol, (a) crystal b->d) liquid—supercooled liquid—glass (c) super-cooled liquid, extrapolation assuming very slow transformation to glass.

CAS 24800-44-0. H0(C3H60)2C3H60H. Properties Colorless liquid. Supercools instead of freezing, bp 268C, d 1.019 (25/25C), bulk d 8.51 lb/ gal, refr index 1.442 (25C), flash p 285F (140.5C). Soluble in water, methanol, ether. Combustible. Use Intermediate in resins, plasticizers, pharmaceuticals, insecticides, dyestuffs, mold lubricants. 

Figure 2.2. The van der Waals-type phase diagram for one mole of argon. C = 150 K is the critical point, TP is the triple point line of the coexistence between solid, liquid and vapor. The upper shaded area represents the liquid-vapor coexistence, while the lower that of solid-vapor. Vapor exists on the right hand side of the shaded areas, while liquid and solids on their left. The supercritical region is that above the critical point, where (at high pressures) the vapor density is comparable to that of liquid. Supercooled vapor is also indicated by a series of solid points. After [Flowers and Mendoza, 1970].

Crystallization (film preparation) CrystaUization of polymorphs from the melt (liquid, supercooled) Crystal growth characteristics (melt, solution) Crystal growUi kinetics MorjAiology of crystals... 

The dilatation of a fat is the isothermal expansion (due to the transition from the solid to the liquid state) of the fat previously solidified under well-defined conditions. The dilatation indicates therefore the difference between the volume the fat would occupy at the measuring temperature if it were completely liquid (supercooled) and the actual volume of the fat at this temperature. 

The phenomenon of expulsion and adherence of excess drug in a liquid supercooled state on the surface of solid lipid nanoparticles at higher drug load was already described by Bunjes et al. on tripalmitin nanoparticles loaded with ubidecarenone. ... 

In order to understand why liquid water is so unusual, it seems instructive to look at the phase behavior of water at subzero temperatures. Figure 1 shows schematically the regions in the P- Tplane where water is found as a stable liquid, supercooled liquid (metastable), and glass or amorphous ice (metastable). Liquid water is the stable phase above the melting temperature m(/). Below Tm P), the stable phase of water is ice the particular stable ice phase depends on pressure and temperature (see Figure 2). For clarity, the different ice phases are not indicated in Figure 1. 

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